lecture 5.105 Amino acids

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Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 1 WHEN WE ENDED LAST TIME WE HAD JUST LISTED THE THINGS THAT PROTEINS DO What is it about proteins that allows them to have all these properties and more? Proteins are linear polymers of building blocks called amino acids. Their properties depend entirely on the collective properties of the amino acids in a protein, and the order in which they are there. This sets the 3D shape of the protein. So, we need to understand something of the properties of amino acids. Amino acids have the general structure: Amino acids never have this form in solution. Why not? Look at the simplest amino acid, glycine (R = H). Its different forms are in equilibrium We will examine their acid/base properties later. Amino acids have chiral centers; that is, they are asymmetric. They can exist as stereoisomers.
Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 2 The isomers are categorized with reference to glyceraldehyde, the simplest sugar to have an asymmetric C atom. All amino acids in proteins are L stereoisomers. This arises from the exquisite sensitivity of the active sites of enzymes to 3d structures. D-amino acids occur in nature, but not in proteins. The building blocks of proteins are hooked together via the peptide bond . Because the peptide bond has partial double bond character , it is planar .
Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 3 This imparts some important properties to proteins, which we will see later. Since amino acids all have the amino and carboxyl groups, the peptide bond can, in principle, be formed in either direction. This is why proteins are linear polymers of amino acids joined by peptide bonds. Recall the general structure of an amino acid in the neutral pH form: Proteins are made from 20 different L-amino acids. The amino acids can be grouped together in many different ways, and we'll go through the using the grouping from Lehninger. In order to facilitate writing them down, amino acids have been given abbreviations. There are individual three-letter and one-letter abbreviations, which you must learn. For instance, Glycine is abbreviated Gly or G. Not always easy. For instance, Glutamine is abbreviated Gln or Q. I will give you the long, three letter abbrev and the one letter abbrev. I will also give you a number that corresponds to the hydrophobicity of the amino acid. There are a couple of scales that can be used, and I’ll just pick one. In this scale, plus = hydrophobic and negative = hydrophilic. Scale goes from +4.5 (Ile) to -4.5 (Arg). Think of it as related to the change in Gibbs free energy in moving the amino acid from non-polar solvent (acetone) to water. Draw bar to the far right. GROUP 1; NON-POLAR, ALIPHATIC (OFTEN HYDROPHOBIC) G,A,V,L,I,P
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Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 4 Glycine; Gly, G, 0.4 Smallest amino acid. Not terribly hydrophobic. No acid/base groups, no potential H- bonding groups, not especially reactive. Alanine; Ala, A, 1.8 Properties much like glycine, but more hydrophobic. Valine; Val, V, 4.2 "V-shaped". Very hydrophobic. Leucine; Leu, L 3.8 "Like val only Longer". Hydrophobic. Isoleucine; Ile, I 4.5 "Isomer of leucine". Most hydrophobic of all amino acids. Proline; Pro, P -1.6 The only cyclic amino acid. Somewhat hydrophilic. Constrained movement around peptide bond; puts kink in proteins; we'll discuss this point later. GROUP 2; POLAR, UNCHARGED S,T,C,M,N,Q
Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 5 Serine; Ser, S -0.8 Not charged, but polar because of OH group; good hydrogen bonder; often in active sites because good e - -phile. pK a not in the physiol. pH range, not deprotonated under normal circumstances. (13.6) Threonine ; Thr, T -0.7 Much like S, but not often at enzyme active site. Cysteine; Cys, C 2.5 Sort of a Ser analog, but not so good a H-bonder because electronegativity of O > that of S. pK a beyond physiol pH range. (10.3) The S can be oxidized, and then linked to another to form a disulfide bridge. In this configuration, it is called Cystine. Can hook distant portions of a protein together, extremely important in stabilizing protein structure. Can be reduced to two Cys's again. Methionine, Met, M , +1.9 Called "thiol-like". Always the first amino acid added to start protein synthesis, initiator codon (often removed in eukaryotes, modified in prokaryotes). Hydrophobic. Asparagine, Asn, N , -3.5 Amine of aspartate (we'll see). Good H-bonder. Not a nucleophile of acid/base because the e - is shared by the O and N.
Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 6 Glutamine, Gln, Q , -3.5 Similar properties as Asn GROUP 3; AROMATIC F,Y,W Phenylalanine; Phe, F , 2.8 V. hydrophobic. Large and bulky. Strong UV absorber; more on this in a minute. Tyrosine; Tyr, Y , -1.3 V. active side group. Strong H-bonder. Acid/base properties, pK a = 10.1. pK a beyond physiol pH range. Tryptophan; Trp, W , -0.9 Largest amino acid; rarest. Heterocyclic. Does not deprotonate, but does H-bond. Beer's Law - Relating Absorbance to Concentration A technique used very often in the lab is to measure the absorbance of a compound at a particular wavelength, and then to use that to calculate the compound's concentration. A = -log(I out /I in ) Put in wavelength; A = log(I (in) /I (out) ) Beer's Law; A = c d Definitions: (Put on different place on board that can be saved) = wavelength I in , I out = light intensity going in, coming out. A = absorbance at c = concentration in whatever units d = distance across the light path; usually = 1 cm = extinction coefficient; units of conc -1 dist -1
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Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 7 Useful form is: c = A / , when d = 1 cm W and Y have very intense UV absorbencies; high 280 . Can estimate the concentration of a solution of proteins by measuring A 280 and using 280 = 1 (mg/ml) -1 cm -1 . Only an estimate. Can also use this UV absorbance as a marker for the presence of protein. We'll see this when we talk about column chromatography. Question (to come at break with clicker): You have a protein in solution, and you want its concentration. You place 10 l of protein solution into a cuvette with 990 l H 2 O, and measure A 280 = 0.032. What concentration? GROUP 4; NEGATIVELY CHARGED, ACIDIC D,E Aspartate; Asp, D , -3.5 (Aspartic acid). Usually ionized, pK a = 3.9. V. hydrophilic. Found in active sites. Participates in salt bridges, H-bonds. Glutamate; Glu, E , -3.5 (Glutamic acid). Properties similar to Asp. pK a = 4.2
Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 8 GROUP 5; POSITIVELY CHARGED, BASIC K,R,H H Lysine; Lys, K , -3.9 Protonated at physiol. pH, pK a = 10.5. Often in active sites. Good H-bonder, salt bridge Arginine; Arg, R , -4.5 pK a = 12.5. H-bonds, salt bridges. Most hydrophilic. Histidine; His, H , -3.2 pK a = 6.0. Imidazole group makes only buffer at physiol pH. Important in active sites, but relatively rare. That’s all of them.
Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 9 I will show you how to work a couple of problems concerning the acid/base properties of amino acids. 1. What is the pH of 0.1 M monosodium glutamate? Ans: What are the different types of glutamate? What are the charges? Start with the most acidic form The name tells you that there is one Na + balancing a - charge in glutamate. So you are starting with the third species from the left. Since this compound is amphoteric, pH = ½ (pK a2 + pK a3 ) = ½ (4.2 + 9.7) = 6.95 2. What is the pH of isoelectric glutamic acid? Ans: Start with the uncharged form, second from the left. pH = ½ (2.2 + 4.2) = 3.2
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Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 10 Amino acids have different charges depending on their state of ionization, that is, depending on the pH. Isoelectric point when charge = 0. 3. Which amino acid has the lower isoelectric point, E or K? Ans: So which one has the lower isoelectric point? ½ (2.2 + 4.2) = 3.2 < ½ (9.0 + 10.5) = 9.75 4. What is the net charge of glutamate at pH 4.8? Ans: You need to calculate the amount of the differently charged species present at pH 4.8. [+1] = 0, too far away from the pK a for it to be present in significant amounts. Similarly, [-2] = 0. What are the concentrations of [0] and [-1]? Use Henderson-Hasselbalch eqn. 4.8 = 4.2 + log([A - ]/[HA]), 0.6 = log([A - ]/[HA]), 10 0.6 = [A - ]/[HA] = 4.0 [A - ] = 4 • [HA] [A - ] + [HA] = 100% = 1.0 = 4 • [HA] + [HA] = 5 • [HA] 5[HA] = 1,
Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 11 [HA] = 1/5 = 0.2, [A - ] = 0.8 Total charge = 0.2 • [0] + 0.8 • [ -1] = -0.8 5. Calculate pI of glutamate. Ans: You want to know the pH at which most of the glutamate is in the AA 0 form. At that pH, since the AA 0 form undergoes a disproportionation reaction, the concentration of AA -1 and AA +1 are the same. This then becomes the same question as: What is the pH of a solution to which you've added AA 0 ? The answer is 1/ 2 (pK a1 + pK a2 ). For glutamate, the AA 0 is the second form from the left. So pI = 3.2. 6. What is the pI of Histidine? Ans: Write the structures from most acidic to most basic 1.8 6.0 9.2 AA +2 AA +1 AA 0 AA -1 ; pK a s are 1.8, 6.0 and 9.2. Where is the neutral form? What pK a s apply? 6.0 and 9.2 So the pI = ½ (6.0 + 9.2) = 7.6 7. What is the pI of the peptide G-K-A? The pK a s are as follows: for -COOH, 2.34; for -NH2, 9.60; for -NH2, 10.53 Ans:
Biological Sciences 105 Lecture 5, October 1, 2018 Copyright Steven M. Theg, 2087. All federal and state copyrights reserved for all original material presented in this course through any medium, including lecture or print. 12 When a peptide bond is formed, the Ns and Cs involved are no longer available for titration. So they drop out of the problem. Only the N-terminus of G, the C-terminus of A and the -amine of K are part of the charge/pH calculation. Write the peptide from N to C terminus, and then from most acidic on left to most basic on right. Look at the charge on the different species. Define pI as the isoelectric point, the pH at which there is no charge. This applies to peptides as well as AAs. The sequence of amino acids in a protein is called the protein’s primary structure. This forms the backbone of the protein. It is always written N-terminus to C-terminus. SOME EQUATIONS YOU’VE HAD THAT YOU SHOULD MEMORIZE ΔG = ΔH - TΔS ΔG°’ = - RTlnKeq ΔG = ΔG°’ + RTln{[products]/[reactants]} pH = pKa + log{[A-]/[HA]} Please do the practice problems.
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